For the following equilibrium reactionthe equilibrium concentr

Question

For the following equilibrium reaction

$2SO_{2}(g)+o_{2}(g)\rightleftharpoons 2so_{3}(g)K_{c}=245(at\;100\;K)$

the equilibrium concentrations are [SO₂]=0.204,[O₂]=0.0264 and [SO₃]=0.368. Show that the equilibrium will shift towards the reactants side if the concentration of SO₂ is suddenly doubled.

23 Jan 2025

Answer :

Word Count : 311

To determine whether the equilibrium will shift towards the reactants' side when the concentration of SO₂ is doubled, we compare the reaction quotient $ Q_c $ with the equilibrium constant $ K_c $. ### Step 1: Write the Expression for $ K_c $ For the reaction: \[ 2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) \] The equilibrium constant expression is: \[ K_c = \frac{[SO_3]^2}{[SO_2]^2 [O_2]} \] Given that $ K_c = 245 $ at 100 K, and the equilibrium ___ _____ _____ ________ __________ _____ ________ __________ ____ ___ ____ ___.
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